4. An atom is neutral because it has the same number of protons as it has:electrons
O neutrons
O Neither... An atom isn't neutral!

Answers

Answer 1

Answer:

Taking into account the constitution of an atom, an atom is neutral because it has the same number of protons as it has electrons.

Constitution of an atom

An atom is the smallest constituent unit of ordinary matter that has the properties of a chemical element.

Every atom consists of a nucleus in which neutrons and protons meet and energy levels where electrons are located.

The neutron is an electrically neutral subatomic particle, while the proton has a positive electrical charge. Electrons have a negative charge, move around the nucleus at different energy levels and are attracted to protons, positive in the atom through electromagnetic force.

Atomelectrically neutral

An atom is considered electrically neutral when it has the same number of positive and negative charges. That is, an electrically neutral atom has the same number of protons (with a positive charge) and electrons (with a negative charge).

In summary, an atom is neutral because it has the same number of protons as it has electrons.

Learn more about atomelectrically neutral:

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Answer 2

Answer: Neutrons the way this question is setup the atom would not be able to be neutral

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The vapor pressure of liquid octane, C8H18, is 100 mm Hg at 339 K. A sample of C8H18 is placed in a closed, evacuated 537 mL container at a temperature of 339 K. It is found that all of the C8H18 is in the vapor phase and that the pressure is 68.0 mm Hg. If the volume of the container is reduced to 338 mL at constant temperature, which of the following statements are correct?a. No condensation will occur.
b. Some of the vapor initially present will condense.
c. The pressure in the container will be 100. mm Hg.
d. Only octane vapor will be present.
e. Liquid octane will be present.

Answers

Answer:

the final pressure (108.03 mmHg ) inside the container at 339 K is more than the vapor pressure of liquid octane (100 mmHg) at 339 K.

Hence,

b. Some of the vapor initially present will condense.

e. Liquid octane will be present.

Explanation:

Given that;

The vapor pressure of liquid octane, C8H18, is 100 mm Hg at 339 K

Initial volume of the container, V1 = 537 mL

Initial vapor pressure, P1 = 68.0 mmHg

Final volume of the container, V2 = 338 mL

Let us say that the final vapor pressure = P2

From Boyle's law,

P2V2 = P1V1

P2 * 338 = 68.0 * 537

338P2 = 36516

P2 = 36516 / 338

P2 = 108.03 mmHg

Thus, the final pressure (108.03 mmHg ) inside the container at 339 K is more than the vapor pressure of liquid octane (100 mmHg) at 339 K.

Hence,

b. Some of the vapor initially present will condense.

e. Liquid octane will be present.

Classify these bonds as ionic, polar covalent, or nonpolar covalent p cl k br c c

Answers

Types of Bonds can be predicted by calculating the difference in electronegativity.
If, Electronegativity difference is,

Less than 0.4 then it is Non Polar Covalent

Between 0.4 and 1.7 then it is Polar Covalent

Greater than 1.7 then it is Ionic

For P and Cl,
E.N of Chlorine    = 3.16
E.N of Phosphorous = 2.19
   ________

E.N Difference 0.97 (Polar Covalent)

For K and Br,
E.N of Bromine      = 2.96
E.N of Potassium    = 0.82
   ________

E.N Difference 2.14 (Ionic)

For C and C,
E.N of Carbon      = 2.55
E.N of Carbon     = 2.55
   ________

E.N Difference 0.00 (Non-Polar Covalent)

Which unit would be most appropriate for measuring the volume of water in a swimming pool? Liters or Kiloliters

Answers

The most appropriate for measuring the volume of water in a swimming pool is kilolitres.

Consider a pool that is 25 m long by 10 m wide with an average depth of 1.5 m.

V = lwh = 25 m × 10 m × 1.5 m = 375 m³

1 L = 1 dm³, so

V = 375 m³ × (10 dm/1 m)³ = 375 000 dm³ = 375 000 L = 375 kL

Thus, the cubic metre or kilolitre is more appropriate, because it gives more manageable numbers (i.e., between 0.1 and 1000)

Calculate the pH of a solution prepared by adding 20.0 mL of 0.100 M HCl to 80.0 mL of a buffer that is comprised of 0.25 M C2H5NH2 and 0.25 M C2H5NH3Cl. Kb of C2H5NH2 = 9.5 x 10-4.

Answers

Answer: The pH of resulting solution is 10.893

Explanation:

To calculate the number of moles for given molarity, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}* 1000}{\text{Volume of solution (in mL)}}$

For ethylamine:

Molarity of ethylamine solution = 0.25 M

Volume of solution = 80 mL

Putting values in above equation, we get:

$0.25M=\frac{\text{Moles of ethylamine}* 1000}{80mL}\n\n\text{Moles of ethylamine}=(0.25* 80)/(1000)=0.02mol$

For HCl:

Molarity of HCl = 0.100 M

Volume of solution = 20.0 mL

Putting values in above equation, we get:

$0.100M=\frac{\text{Moles of HCl}* 1000}{20.0mL}\n\n\text{Moles of HCl}=(0.100* 20)/(1000)=0.002mol$

For $C_2H_5NH_3Cl$ :

Molarity of $C_2H_5NH_3Cl$ solution = 0.25 M

Volume of solution = 80 mL

Putting values in above equation, we get:

$0.25M=\frac{\text{Moles of }C_2H_5NH_3Cl* 1000}{80mL}\n\n\text{Moles of }=(0.25* 80)/(1000)=0.02mol$

The chemical reaction for ethylamine and HCl follows the equation:

$C_2H_5NH_2+HCl\rightarrow C_2H_5NH_3Cl$

Initial: 0.02 0.002 0.02

Final: 0.018 - 0.022

Volume of solution = 20.0 + 80.0 = 100 mL = 0.100 L (Conversion factor: 1 L = 1000 mL)

To calculate the pOH of basic buffer, we use the equation given by Henderson Hasselbalch:

$pOH=pK_b+\log(([salt])/([base]))$

$pOH=pK_b+\log(([C_2H_5NH_3Cl])/([C_2H_5NH_2]))$

We are given:

$pK_b$ = negative logarithm of base dissociation constant of ethylamine = $-\log(9.5* 10^(-4))=3.02$

$[C_2H_5NH_3Cl]=(0.022)/(0.100)$

$[C_2H_5NH_2]=(0.018)/(0.100)$

pOH = ?

Putting values in above equation, we get:

$pOH=3.02+\log((0.022/0.100)/(0.018/0.100))\n\npOH=3.107$

To calculate pH of the solution, we use the equation:

$pH+pOH=14\npH=14-3.107=10.893$

Hence, the pH of the solution is 10.893

The pH of the solution is 10.9

Data;

Volume of buffer = 80mL
Volume of HCL = 20.0mL
conc. of C2H5NH2 = 0.25M
conc. of C2H5NH3Cl = 0.25
Kb of C2H5NH2 = 9.5*10^-4

pH of a Solution

The pH of buffer can be calculated by using Henderson-Hasselbalch's equation

$pOH = _pKb+ log ([salt])/([base])$

The initial moles of salt present is calculated as

$0.25 * 80*10^-^3 = 0.02mmoles$

The initial moles of base present is calculated as

$0.25*80*10^-^3 = 20mmoles$

On adding HCl the following reaction will occurs

$C_2H_5NH_2 + HCl \to C_2H_5NH_3Cl$

This will lead to formation of extra moles of salt that is equal to moles of acid added and eventually lead to decrease in number of moles of base by equal measure.

Moles of HCl added is

$moles of HCL= 0.1 * 20 * 10^-^3 = 2mmoles$

Adding the value

Moles of salt present = 20 + 2 = 22mmoles

Subtracting the value

Moles of base left = 20-2 = 18mmoles

Now using Henderson-Hasselbalch's equation we can calculate the pOH of solution

$pKb = -logKb = -log (9.5*10^-^4) = 3.02$

The pOH of the base can be calculated as

$pOH = 3.02 + log ((22)/(18)) = 3.107$

Using the above, we can solve for the pH of the solution.

$pH = 14 - pOH = 10.893$

The pH of the solution is 10.9

Learn more on pH of a solution using Henderson-Hasselbalch equation here;

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What is the solubility of substance?

Answers

Explanation:

Solubility is a chemical property referring to the ability for a given substance, the solute, to dissolve in a solvent. It is measured in terms of the maximum amount of solute dissolved in a solvent at equilibrium. The resulting solution is called a saturated solution.

In metallic bonds, the mobile electrons surrounding the positive ions are called a(n)